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Question

Statement 1: AgI is less soluble in water than AgF due to more polarization of I− ion in comparison to F− ion.
Statement 2: The melting point of BaCl2 is higher than the melting point of BeCl2 due to the greater ionic nature of BaCl2.
Statement 3: The order of hydrated radii is: Al3+(aq)>Mg2+(aq)>Na+(aq)

A
T T T
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B
T T F
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C
T F T
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D
F T T
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Solution

The correct option is A T T T
As I is larger in size than F, the polarisability of I is greater than that of F and AgF shows less covalent character thus more soluble in polar solvents.
Smaller the cation, more is the covalent character. Thus BaCl2 is less covalent (more ionic) than BeCl2 due to larger size of Ba2+ and will be having higher melting point.
Smaller the cation more will be the extent of hydration. The order for the size is: Al3+<Mg2+<Na+. Hence, the order of hydrated radii will be just reverse, i.e., Al3+(aq)>Mg2+(aq)>Na+(aq)

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